Answer:
95.41°C
Explanation:
T1 = 56.5°C = 329.65K
∇Hᵥₐ = 31.3kJ/mol
p2 = 226mmHg = 0.301bar
p1 = 1bar
R = ideal gas constant = 0.008314kJ/Mol.K
From definition, the normal boiling point is at 1 bar which relates to Clausius-Clapeyron equation relates to vapour pressure to temperature.
In(P₂/P₁) = -∇Hᵥₐ /R (1/T₂ - 1/T₁)
solving for T₂,
R / ∇Hᵥₐ . In(P₂/P₁) = 1/T₂ - 1/T₁
1/T₂ = 1/T₁ - R / ∇Hᵥₐ * In(P₂/P₁)
1/T₂ = (1 / 329.65) - (0.008314 / 31.3) In (0.30 / 1)
1/T₂ = (3.033*10⁻³) - (2.656*10⁻⁴ * -1.204)
1/T₂ = 3.033*10⁻³ - 3.197*10⁻⁴
1/T₂ = 2.713*10⁻³
T₂ = 368.56K
T2 = 95.41°C
